Chapter 5, Problem 5.98P

Interpretation Introduction

(a)

Interpretation:

The limiting reactant for reaction ${\text{2NO + O}}_2\to 2{\text{ NO}}_2$ given that 2.0 mol of NO and 1.1 mol of ${\text{O}}_2$ are involved should be determined.

Concept Introduction:

When the reaction takes place, products are formed. But the amount of product formed depends on the reactants. If the reaction stops abruptly it means that one of the reactants is not enough for the product formation. Such a reactant is termed as limiting reactant.

Interpretation Introduction

(b)

Interpretation:

The limiting reactant for reaction ${\text{2NO + O}}_2\to 2{\text{ NO}}_2$ given that 4.2 mol of NO and 2.0 mol of ${\text{O}}_2$ are involved should be determined.

Concept Introduction:

If a reaction stops abruptly, it means that there is not enough of a particular reactant for the chemical reaction to take place. In such a condition, such a reactant is called as limiting reactant as this reactant is required for the reaction to complete.

Interpretation Introduction

(c)

Interpretation:

The limiting reactant for reaction ${\text{2NO + O}}_2\to 2{\text{ NO}}_2$ given that 15 g of NO and 10 g of ${\text{O}}_2$ are involved should be determined.

Concept Introduction:

For reaction to be complete and product to be formed, one of the reactants should be enough to get the result. This reactant is said to be the limit reactant. Sometimes, the other reactant which is in excess is excess reagent.

Interpretation Introduction

(d)

Interpretation:

The limiting reactant for reaction ${\text{2NO + O}}_2\to 2{\text{ NO}}_2$ given that 10 g of NO and 4g of ${\text{O}}_2$ are involved should be determined.

Concept Introduction:

A reaction is said to be complete when products are formed from reactants involved. But if reaction stops abruptly, then it is said that one of the reactant is not enough for the completion. This reactant is then said to be limiting reactant.